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The problem asks to calculate the pH of a solution where 652 mg of pure nitric acid (HNO₃) is dissolved in enough water to make 340 mL of solution. Let's go step by step to find the pH.

### Step 1: Molar mass of Nitric Acid (HNO₃)
The molar mass of HNO₃ is calculated as follows:
- H: 1 g/mol
- N: 14 g/mol
- O₃: 16 × 3 = 48 g/mol

So, the total molar mass of HNO₃ = 1 + 14 + 48 = **63 g/mol**.

### Step 2: Convert mass of HNO₃ to moles
We have 652 mg of HNO₃, which is equal to 0.652 g. To convert grams to moles, use the formula:

\[
\text{moles of HNO₃} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}}
\]

\[
\text{moles of HNO₃} = \frac{0.652}{63} = 0.01035 \text{ mol}
\]

### Step 3: Calculate the concentration of HNO₃
The concentration of HNO₃ is given by:

\[
\text{Concentration (M)} = \frac{\text{moles of HNO₃}}{\text{volume of solution (L)}}
\]

The volume is 340 mL, which is 0.340 L. Therefore,

\[
\text{Concentration} = \frac{0.01035}{0.340} = 0.03044 \text{ M}
\]

### Step 4: pH calculation
Since HNO₃ is a strong acid, it fully dissociates in water, meaning the concentration of H⁺ ions is the same as the concentration of HNO₃. Therefore:

\[
[\text{H}^+] = 0.03044 \text{ M}
\]

The pH is calculated using the formula:

\[
\text{pH} = -\log[\text{H}^+]
\]

\[
\text{pH} = -\log(0.03044) \approx 1.52
\]

### Final Answer:
The pH of the solution is approximately **1.52**.

---

Would you like any further details or clarifications on the process?

### Follow-up questions:
1. What is the significance of the molar mass in calculating concentration?
2. How does full dissociation of strong acids like HNO₃ affect pH?
3. What would happen if nitric acid only partially dissociated?
4. How can you calculate the concentration if the volume of the solution changes?
5. How does temperature affect pH calculations in strong acids?

### Tip:
Always check the dissociation behavior of the acid before calculating the pH—strong acids dissociate fully, which simplifies the calculation.

A chemist dissolves 652 mg of pure nitric acid in enough water to make up 340 mL of solution. Calculate the pH of the solution. Be sure your answer has the correct number of significant digits.

Learn how to calculate the pH of a solution where 652 mg of pure nitric acid (HNO₃) is dissolved in enough water to make 340 mL of solution. The solution covers concepts such as molar mass, moles, concentration, and pH calculations for a strong acid. Suitable for college-level chemistry.

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